An aqueous solution of an unknown solid salt was placed into fivedifferent test tubes. Into each test tube a couple of drops of differentindicators were then added to each test tube and the color of theindicator in the solution was recorded as shown below. What is theapproximate pH of the solution?TestpHAcidBaseColor in UnknownIndicatortubeRange ColorColorSolution3.0 -1Methyl orange4.4RedYellowYellow3.0 -Congo RedPurpleRedRed5.0Bromcresol3.8 -YellowBlueBlueGreen5.4Bromthymol6.0 -7.64YellowBlueYellowBlue8.2 -PhenolphthaleinColorless BlueColorless10.04.3O 8.4O 5.26.7

The approximately pH value would be 5.2

An aqueous solution of an unknown solid salt was placed into five different test tubes. Into each test tube a couple of drops of different indicators were then added to each test tube and the color of the indicator in the solution was recorded as shown below. What is the approximate pH of the solution? Acid Base Color in Unknown Test Indicator tube pH Range Color Color Solution 3.0 - Methyl orange 4.4 Red Yellow Yellow 1 3.0 - Congo Red Purple Red Red 5.0 Bromcresol 3.8 - Yellow Blue Blue Green 5.4 Bromthymol 4 Blue 6.0 - Yellow Blue Yellow 7.6 8.2 - Phenolphthalein 10.0 Colorless Blue Colorless LO

An aqueous solution of an unknown solid salt was placed into five different test tubes. Into each test tube a couple of drops of different indicators were then added to each test tube and the color of the indicator in the solution was recorded as shown below. What is the approximate pH of the solution? Acid Base Color in Unknown Test Indicator tube pH Range Color Color Solution 3.0 - Methyl orange 4.4 Red Yellow Yellow 1 3.0 - Congo Red Purple Red Red 5.0 Bromcresol 3.8 - Yellow Blue Blue Green 5.4 Bromthymol 4 Blue 6.0 - Yellow Blue Yellow 7.6 8.2 - Phenolphthalein 10.0 Colorless Blue Colorless LO

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Which of the following is true of a buffer solution that contains equivalent amounts of acid and conjugate base? The pH will always be greater than 7, regardless of the acid and conjugate base. The pH of the solution will be equal to the pKa of the acid. The pH of the solution will be equal to Kw. The pH will be equal to the concentration of the conjugate base. The pH will be equal to the concentration of the acid.
Use the References to access important values if needed for this question. Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.17 M hydrocyanic acid + 0.19 M sodium cyanide 0.21 M perchloric acid + 0.18 M potassium perchlorate 0.28 M ammonia + 0.33 M ammonium bromide 0.18 M barium hydroxide + 0.22 M barium bromide 0.35 M calcium nitrate + 0.22 M calcium chloride
Equimolar quantities of lithium hypochlorite and hypochlorous acid are placed into solution. What happens to the buffer system if some sodium hydroxide is added to the solution? ) The sodium hydroxide reacts with the hypochlorite ion and the pH decreases significantly. The sodium hydroxide reacts with the hypochlorious acid and the pH increases significantly. The sodium hydroxide reacts with the hypochlorite ion and the pH decreases only slightly. The sodium hydroxide reacts with the hypochlorious acid and the pH increases only slightly.
What is the general composition of a buffer and in your own words explain why it resists change in PH.
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Write the color of indicators and its pH ranges. pH = 1.0 pH = 14.0 Phenolphthalein Methyl Orange Methyl Red
An unknown solution is blue with indigo carmine and blue with thymolphthalein. From that information, predict the approximate pH range of the unknown solution, then determine the colour of the following indicators in that solution. Indicator Colour alizarin yellow R yellow/red/orange phenolphthalein colourless/pink thymol blue yellow/red/orange/green/blue
Use the following information as a guide to help answer the next three questions. Your answer MUST be in the same format. Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between .0 and 7.6 6. Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Using the method outlined above in the example of bromothymol blue, indicate what the colours of the indicators tell us about the pH approximation of the solution. Values and wording are very important, so be precise. Be sure to word your pH approximation as outlined in the example. Indicator Colour pH approximation methyl red orange Indicator Colour pH approximation phenolphthalein colourless Indicator Colour pH approximation phenol red red
Select ALL of the following that can be determined from the titration of a strong, monoprotic acid with a standardized solution of sodium hydroxide? moles of acid in the titration moles of hydroxide ions used in the titration mass of acid titrated | volume of sodium hydroxide used in the titration Select ALL of the following quantities that must be used in a titration calculation to find the identity of an unknown strong acid: concentration of the standardized base solution stoichiometric ratio of acid to base volume of the acid solution used in the titration volume of the base used in the titration at the equivalence point Need Help?
Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between 6.0 and 7.6 Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Indicator Colour pH approximation orange IV orange Indicator Colour pH approximation thymol blue red Indicator Colour pH approximation alizarin yellow R red
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Use an example to discuss how a buffer solution resists changes in pH when small amounts of acid or base are added.